Complete Ionic Equations. Reactants: Zn + I 2 Product: Zn I 2.

Complete Ionic EquationsComplete Ionic Equations


Reactants: Zn + IReactants: Zn + I22 Product: Zn IProduct: Zn I22

Murphy's LawsMurphy's Lawsofof

Science and TechnologyScience and Technology

Any instrument when dropped will roll into the least accessible corner.

Complete Ionic Equations:Complete Ionic Equations:At the conclusion of our time together, At the conclusion of our time together,

you should be able to:you should be able to:

1.1. Define molecular, complete and net ionic Define molecular, complete and net ionic equationsequations

2.2. Write molecular, complete and net ionic Write molecular, complete and net ionic equationsequations

3.3. Identify a neutralization reactionIdentify a neutralization reaction4.4. Realize that this is one of the 5 basic Realize that this is one of the 5 basic

types of chemical reactionstypes of chemical reactions

Double Replacement ReactionsDouble Replacement Reactions

• Double Replacement Reactions Double Replacement Reactions occur when occur when a metal replaces a metal in a compound and a a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compoundnonmetal replaces a nonmetal in a compound

• Compound + compound Compound + compound compound+ compound+ compoundcompound

• AB + CD AB + CD AD + CB AD + CB

Double Replacement ReactionsDouble Replacement Reactions

• Think about it like “foil”ing in algebra, first and Think about it like “foil”ing in algebra, first and last ions go together + inside ions go togetherlast ions go together + inside ions go together

• Example:Example:

AgNOAgNO3(aq) 3(aq) + NaCl+ NaCl(s) (s) AgCl AgCl(s) (s) + NaNO+ NaNO3(aq)3(aq)

• Another example:Another example:

KK22SOSO4(aq) 4(aq) + Ba(NO+ Ba(NO33))2(aq) 2(aq) KNO KNO3(aq)3(aq) + BaSO + BaSO4(s) 4(s) 2

3 Driving Forces for Double Replacement 3 Driving Forces for Double Replacement ReactionsReactions

• Water Forms• Gas Forms• Solid Forms• If one of the above is not a

product, there will be no reaction.

PracticePractice

• Predict the products. Balance the equationPredict the products. Balance the equation

1.1. HClHCl(aq)(aq) + AgNO + AgNO33(aq) (aq)

2.2. CaClCaCl22(aq) (aq) + Na+ Na33POPO4 (aq) 4 (aq)

3.3. Pb(NOPb(NO33)) 2(aq) 2(aq) + BaCl+ BaCl2 (aq) 2 (aq)

4.4. FeClFeCl3 (aq) 3 (aq) + NaOH+ NaOH(aq) (aq)

5.5. HH22SOSO44(aq)(aq) + NaOH + NaOH(aq)(aq)

6.6. KOHKOH(aq)(aq) + CuSO + CuSO4 (aq) 4 (aq)

7.7. Ba(NOBa(NO33)) 2(aq) 2(aq) + K+ K22CrOCrO4 (aq) 4 (aq)

8.8. Demo Time!! Demo Time!!

AgCl + HNO3

NaCl + Ca3 (PO4) 2

Ba(NO3) 2 + PbCl2NaCl + Fe(OH) 3

Na2SO4 + H2O

Cu(OH) 2 + K2SO4

BaCrO4 + KNO3


Once you write the molecular equation Once you write the molecular equation (synthesis, decomposition, etc.), you (synthesis, decomposition, etc.), you should check for reactants and products should check for reactants and products that are soluble or insoluble.that are soluble or insoluble.

We usually assume the reaction is in waterWe usually assume the reaction is in water We can use a solubility table to tell us We can use a solubility table to tell us

what compounds dissolve in water.what compounds dissolve in water. If the compound is soluble (does dissolve If the compound is soluble (does dissolve

in water), then split the compound into its in water), then split the compound into its component ionscomponent ions

If the compound is insoluble (does NOT If the compound is insoluble (does NOT dissolve in water), then it remains as a dissolve in water), then it remains as a compoundcompound

Solubility TableSolubility Table

Solubilities Not on the Table!Solubilities Not on the Table!

Gases will only slightly dissolve in waterGases will only slightly dissolve in water Strong acids and bases dissolve in waterStrong acids and bases dissolve in water

Hydrochloric, Hydrobromic, Hydroiodic, Hydrochloric, Hydrobromic, Hydroiodic, (All Binaries)(All Binaries) Nitric, Sulfuric, Perchloric AcidsNitric, Sulfuric, Perchloric Acids (Ternary Acids with 2 more O than H)(Ternary Acids with 2 more O than H) Group I hydroxidesGroup I hydroxides

Water slightly dissolves in water! (H+ and Water slightly dissolves in water! (H+ and OH-)OH-)


Molecular Equation:Molecular Equation:

KK22CrOCrO4(aq)4(aq) + Ba(NO + Ba(NO33))2(aq)2(aq) BaCrO BaCrO4(s)4(s) + 2 + 2

KNOKNO3(aq)3(aq)

SolubleSoluble Soluble Insoluble Soluble Soluble Insoluble Soluble

Complete Ionic Equation:Complete Ionic Equation:

2 K2 K++ + CrO + CrO44 -2-2 + Ba+ Ba+2+2 + 2 NO + 2 NO33--

BaCrOBaCrO44 (s) + 2 K (s) + 2 K++ + 2 NO + 2 NO33--

Net Ionic EquationsNet Ionic Equations

These are the same as complete ionic These are the same as complete ionic equations, but you should cancel out ions equations, but you should cancel out ions that appear on BOTH sides of the equationthat appear on BOTH sides of the equation


2 K2 K++ + CrO + CrO44 -2-2 + Ba + Ba+2+2 + 2 NO + 2 NO33--

BaCrOBaCrO44 (s) + 2 K (s) + 2 K++ + 2 + 2 NONO33

--

Net Ionic Equation:Net Ionic Equation:

CrOCrO44 -2-2 + Ba + Ba+2+2 BaCrO BaCrO44 (s) (s)Spectator Ion

Neutralization ReactionNeutralization Reaction

Acid + Base Acid + Base Salt + Water Salt + Water

Molecular Equation:Molecular Equation:

HCl + NaOH HCl + NaOH NaCl + HNaCl + H22OO

SolubleSoluble Soluble Soluble InsolubleSoluble Soluble Insoluble


HH++ + Cl + Cl-- + Na + Na++ + OH + OH-- HH22O (O (ll) + Na) + Na++ + Cl + Cl--

Net Ionic Equation for Net Ionic Equation for Neutralization ReactionsNeutralization Reactions

These are the same as complete ionic These are the same as complete ionic equations, but you should cancel out ions equations, but you should cancel out ions that appear on BOTH sides of the equationthat appear on BOTH sides of the equation


HH++ + Cl + Cl-- + Na + Na++ + OH + OH-- HH22O (O (ll) + Na) + Na++ + Cl + Cl- -

Net Ionic Equation:Net Ionic Equation:

HH++ + OH + OH-- H H22O (O (ll))

Complete Ionic Equations:Complete Ionic Equations:Let’s see if you can:Let’s see if you can:

1.1. Define molecular, complete and net ionic Define molecular, complete and net ionic equationsequations

2.2. Write molecular, complete and net ionic Write molecular, complete and net ionic equationsequations

3.3. Identify a neutralization reactionIdentify a neutralization reaction4.4. Realize that this is one of the 5 basic Realize that this is one of the 5 basic

types of chemical reactionstypes of chemical reactions

Familiar SayingFamiliar Saying

One pyrus malus per diem restrains the arrival of the Hippocratic apostle.

An apple a day keeps the doctor away!!

Practice Quiz Practice Quiz Net Ionic EquationsNet Ionic Equations

Write the molecular, complete ionic, and net Write the molecular, complete ionic, and net ionic equations for this reaction: Silver nitrate ionic equations for this reaction: Silver nitrate reacts with calcium chloridereacts with calcium chloride

Molecular: Molecular:

2AgNO2AgNO33 + CaCl + CaCl22 2AgCl + Ca(NO 2AgCl + Ca(NO33))22

Complete Ionic:Complete Ionic:

2Ag2Ag++ + 2NO + 2NO33--+ Ca+ Ca2+2+ + 2Cl + 2Cl-- 2AgCl + Ca 2AgCl + Ca2+2+ + +

2NO2NO33--

Net Ionic:Net Ionic:

2Ag2Ag++ + + 2Cl2Cl-- 2AgCl 2AgCl

I don’t feel so stupid now…I don’t feel so stupid now…

Complete Ionic Equations. Reactants: Zn + I 2 Product: Zn I 2.

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Transcript of Complete Ionic Equations. Reactants: Zn + I 2 Product: Zn I 2.